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Chemistry > Chapter 12 > Flashcards

Chapter 12 Flashcards

1
Q

Salts can be made by:

A

MCB + A (makes soluble salt)

precipitation (makes insoluble salt)

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2
Q

acid + metal

A

salt + hydrogen gas

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3
Q

acid + carbonate

A

salt + water + carbon dioxide gas

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4
Q

acid + base

A

salt + water

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5
Q

acid + alkali

A

salt + water

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6
Q

zinc (Zn) + hydrochloric acid (HCl)

A

zinc chloride (ZnCl2) + hydrogen gas

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7
Q

copper(II) carbonate (CuCO3) + nitric acid (H2NO4)

A

copper(II) nitrate (Cu(NO3)2) + water + carbon dioxide gas

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8
Q

magnesium oxide (MgO) + sulfuric acid (H2SO4)

A

magnesium sulfate (MgSO4) + water

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9
Q

aqueous ammonia (NH3(aq)) + sulfuric acid (H2NO4)

A

ammonium sulfate ((NH4)2SO4) + water

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10
Q

potassium hydroxide (KOH) + phosphoric acid (H3PO4)

A

potassium phosphate (K3PO4) + water

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11
Q

A salt is a compound formed when a ________ ion or an ________ ion (NH4+) replaces one or more ________ ions of an acid.

A

A salt is a compound formed when a metallic ion or an ammonium ion (NH4+) replaces one or more hydrogen ions of an acid.

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12
Q

zinc hydroxide (Zn(OH2)) + sulfuric acid (H2SO4)

A

zinc sulfate (ZnSO4) + water

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13
Q

Salts that contain water of cyrstallisation are called:

A

hydrated salts

The amount of water crystallised in a hydrated salt is indicated after the . in its chemical formula

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14
Q

Salts that do not contain water of crystallisation are called:

A

anhydrous salts (are often powders, water removed by heating)

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15
Q

Before deciding on how to prepare a salt, you must consider two factors:

A

Is the salt soluble in water?
Soluble salts are prepared by reactions with acids.

Are the starting materials soluble in water?
Insoluble salts are prepared by precipitation reactions.

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16
Q

anhydrous copper(II) sulfate (CuSO4)

A

CuSO4.5H2O

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17
Q

All nitrate salts are

A

soluble

18
Q

All carbonate salts are

A 
insoluble 
except SPA (sodium, potassium, ammonium)
19
Q

All chloride/iodide salts are

A 
soluble
except LS (lead, silver)
20
Q

All sulfate salts are

A 
soluble
except BCL (barium, calcium, lead)
21
Q

Is ammonium phosphate soluble in water?

A

yes

22
Q

Is barium carbonate soluble in water?

A

no

23
Q

Is chromium sulfate soluble in water?

A

yes

24
Q

Is copper(II) nitrate soluble in water?

A

yes

25
Q

Is nickel(II) chloride soluble in water?

A

yes

26
Q

MCB must be in ______, why?

A

MCB must be in excess, because

27
Q

MCB has to be _________ in water, so that the excess starting materials can be removed from the salt solution by __________.

A

MCB has to be insoluble in water, so that the excess starting materials can be removed from the salt solution by filtration.

28
Q

All soluble hydroxides are called alkalis:

A

SPCA (sodium hydroxide, potassium hydroxide, other Group I metal hydroxides, calcium hydroxide (limewater), ammonium hydroxide)

29
Q

All other insoluble hydroxides are called _____.

A

All other insoluble hydroxides are called bases.

30
Q

All oxides are

A

insoluble

except Group I metal oxides (sodium, potassium oxides)

31
Q

Which metals are not suitable for MCB + A?

A

Potassium, sodium and calcium as they react violently with acids.

32
Q

____ does not react well with hydrochloric acid.

A

Lead does not react well with hydrchloric acid.

33
Q

_______ and ______ does not react well with sulfuric acid, why?

A

Calcium and barium does not react well with sulfuric acid, because they produce an insoluble layer.

34
Q

Which metals ar not suitable for MCB + A?

A

Copper and silver as they do not react with dilute acids.

35
Q

How do you increase rate of reaction with acid?

A

By heating up the acid.

36
Q

_______________ is used for substances that easily decompose on heating.

A

Crystallisation is used for substances that easily decompose on heating.

37
Q

_______________ is used for substances that do not decompose on heating.

A

Evaporation to dryness is used for substances that do not decompose on heating.

38
Q

How can you tell if a reaction is complete in titration?

A

An indicator like methyl orange or phenolphtalein will reach endpoint.

39
Q

When do you use titration?

A

When you want to prepare sodium, potassium and ammonium salts. (e.g. NaCl, K2SO4, NH4Cl)

40
Q

Step 1 in titration to prepare sodium nitrate (NaNO3)

A
  1. Fill up a burette with dilute nitric acid. Note the initial burette reading.
41
Q

Step 2 in titration to prepare sodium nitrate (NaNO3)

A
  1. Pipette 25.0cm3 of dilute sodium hydroxide solution into a conical flask.
42
Q

Step 3 in titration to prepare sodium nitrate (NaNO3)

A

3.

Chemistry (3 decks)

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